Nitric acid is a component of acid rain that forms when gaseous nitrogen dioxide pollutant reacts with gaseous oxygen and liquid water to form aqueous nitric acid. Write the balanced chemical equation for this reaction. (Note: this is a simplified representation of this reaction.)

Verified step by step guidance

1. Identify the reactants and products in the reaction: nitrogen dioxide (NO_2), oxygen (O_2), water (H_2O), and nitric acid (HNO_3).
2. Write the unbalanced chemical equation using the chemical formulas: NO_2 (g) + O_2 (g) + H_2O (l) -> HNO_3 (aq).
3. Balance the equation by adjusting coefficients to ensure the same number of each type of atom on both sides of the equation.
4. Start by balancing the nitrogen atoms. There are two nitrogen atoms in 2 NO_2, so you need 2 HNO_3 on the product side.
5. Balance the oxygen atoms. Count the total oxygen atoms on both sides and adjust the coefficients accordingly.

Key Concepts

Chemical Reactions

A chemical reaction involves the transformation of reactants into products through the breaking and forming of chemical bonds. In this context, the reaction between nitrogen dioxide, oxygen, and water leads to the formation of nitric acid. Understanding the types of reactions, such as synthesis and redox reactions, is essential for balancing chemical equations.

Balancing Chemical Equations

Balancing a chemical equation ensures that the number of atoms for each element is the same on both sides of the equation, adhering to the law of conservation of mass. This process involves adjusting coefficients in front of the chemical formulas to achieve balance. It is crucial for accurately representing the stoichiometry of the reaction.

Acid-Base Chemistry

Acid-base chemistry focuses on the properties and reactions of acids and bases. Nitric acid (HNO3) is a strong acid that can dissociate in water to release hydrogen ions (H+). Understanding the behavior of acids in aqueous solutions is important for grasping the implications of acid rain and its environmental effects.